What is the bond of (OClO ) in ClO2-

Options

A. 90
B. 120
C. 105
D. 111

Answer

To determine the bond angle of O-Cl-O in the chlorite ion (ClO2-), we need to analyze the molecular structure and hybridization of the central chlorine atom.

### Step-by-Step Solution:

1. **Identify the Central Atom**:
- In the chlorite ion (ClO2-), chlorine (Cl) is the central atom.

2. **Count Valence Electrons**:
- Chlorine has 7 valence electrons. Each oxygen contributes 6 valence electrons, and we have an additional electron due to the negative charge.
- Total = 7 (Cl) + 2 × 6 (O) + 1 (negative charge) = 20 valence electrons.

3. **Draw the Lewis Structure**:
- Place Cl in the center and bond it to two O atoms.
- Distribute the remaining electrons to satisfy the octet rule for oxygen.
- You will find that Cl forms one double bond with one O and a single bond with the other O, while having two lone pairs of electrons.

4. **Determine Hybridization**:
- The central atom (Cl) has 2 bonded pairs (from the Cl-O bonds) and 2 lone pairs.
- This corresponds to sp3 hybridization (4 regions of electron density).

5. **Consider Lone Pair Repulsion**:
- In sp3 hybridization, the ideal bond angle is 109.5 degrees. However, lone pairs repel more than bonding pairs.
- Since there are 2 lone pairs on Cl, this increases the repulsion and decreases the bond angle.

6. **Calculate the Bond Angle**:
- The bond angle will be less than 109.5 degrees due to the lone pair repulsion.
- Typically, the bond angle in a molecule with 2 lone pairs and 2 bonding pairs is around 105 degrees.

7. **Final Answer**:
- Therefore, the bond angle of O-Cl-O in ClO2- is approximately **105 degrees**.